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A 1.5 L sample of CCl2F2 (g) is held at 56 torr and 23.5 degrees Celsius.?
If the pressure is increased to 150 torr (temp stays the same), what is the new volume of gas?
In the above system, how many grams of CCl2F2 are in the system?
I figured that the new volume of gas is 0.9 L but since the system changes in pressure, I'm not sure how to solve the second question of the problem.
2 Answers
- Roger the MoleLv 74 years agoFavorite Answer
(1.5 L) x (56 torr / 150 torr) = 0.56 L
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n = PV / RT = (56 torr) x (1.5 L) / ((62.36367 L torr/K mol) x (23.5 + 273.15) K) = 0.0045405 mol
(0.0045405 mol) x (120.9135 g CCl2F2/mol) = 0.549 g CCl2F2
- DavidBLv 74 years ago
the mass of the gas does not change, use the ideal gas equation to find the moles of gas at the original pressure. Then calculate the mass from the moles.
PV = nRT so n = PV/RT
